Balance the following the chemical equation

Question

_C2H6+ _O2->_CO2+_H2O

Answer 1

To balance the chemical equation for the combustion of ethane (C₂H₆), we follow these steps:

1. Write the unbalanced equation: \[ \text{C}_2\text{H}_6 + \text{O}_2 \rightarrow \text{CO}_2 + \text{H}_2\text{O} \]

2. Count the number of atoms of each element on both sides.

3. Start by balancing the carbon (C) atoms:

   • There are 2 carbon atoms in C₂H₆, so we need 2 CO₂: \[ \text{C}_2\text{H}_6 + \text{O}_2 \rightarrow 2 \text{CO}_2 + \text{H}_2\text{O} \]

4. Next, balance the hydrogen (H) atoms:

   • There are 6 hydrogen atoms in C₂H₆, so we need 3 H₂O to get 6 hydrogen atoms: \[ \text{C}_2\text{H}_6 + \text{O}_2 \rightarrow 2 \text{CO}_2 + 3 \text{H}_2\text{O} \]

5. Now, count the oxygen (O) atoms on the right side:

   • From 2 CO₂, there are \(2 \times 2 = 4\) oxygen atoms.
   • From 3 H₂O, there are \(3 \times 1 = 3\) oxygen atoms.
   • Total: \(4 + 3 = 7\) oxygen atoms.

6. Now, balance the oxygen (O) on the left side:

   • The O₂ molecule contributes 2 oxygen atoms, so we need \(\frac{7}{2}\) O₂ molecules to get 7 oxygen atoms. To eliminate the fraction, multiply the entire equation by 2: \[ 2 \text{C}_2\text{H}_6 + 7 \text{O}_2 \rightarrow 4 \text{CO}_2 + 6 \text{H}_2\text{O} \]

Now the balanced equation is: \[ \boxed{2 \text{C}_2\text{H}_6 + 7 \text{O}_2 \rightarrow 4 \text{CO}_2 + 6 \text{H}_2\text{O}} \]

Answer 2

Are you positive

Answer 3

Yes, I am confident in the balanced equation provided for the combustion of ethane (C₂H₆). Let's go through the steps once more to ensure everything is clear.

The unbalanced equation is: \[ \text{C}_2\text{H}_6 + \text{O}_2 \rightarrow \text{CO}_2 + \text{H}_2\text{O} \]

Steps to balance it:

1. Balance Carbon (C): There are 2 carbon atoms in C₂H₆, so we need 2 CO₂ on the product side: \[ \text{C}_2\text{H}_6 + \text{O}_2 \rightarrow 2 \text{CO}_2 + \text{H}_2\text{O} \]

2. Balance Hydrogen (H): There are 6 hydrogen atoms in C₂H₆, so we need 3 H₂O on the product side: \[ \text{C}_2\text{H}_6 + \text{O}_2 \rightarrow 2 \text{CO}_2 + 3 \text{H}_2\text{O} \]

3. Count Oxygen (O):

   • From \(2 \text{CO}_2\), we have \(2 \times 2 = 4\) oxygen atoms.
   • From \(3 \text{H}_2\text{O}\), we have \(3 \times 1 = 3\) oxygen atoms.
   • Total oxygen on the right side = \(4 + 3 = 7\) oxygen atoms.

4. Balance Oxygen (O):

   • To get 7 oxygen atoms from O₂, we need \(\frac{7}{2}\) O₂ molecules.
   • This can be rewritten without fractions by multiplying the entire equation by 2: \[ 2 \text{C}_2\text{H}_6 + 7 \text{O}_2 \rightarrow 4 \text{CO}_2 + 6 \text{H}_2\text{O} \]

Thus, the final balanced equation is: \[ \boxed{2 \text{C}_2\text{H}_6 + 7 \text{O}_2 \rightarrow 4 \text{CO}_2 + 6 \text{H}_2\text{O}} \]

If you have any other questions or need further clarification, feel free to ask!